How to describe the electrons defined by the following quantum numbers?
n=3, l=0, #m_l=0#
n=2, l=1 #m_l=1#
Do I just have to say that it has for example one 3s orbital with 3 subshells or do I have to add other information as well? I am struggling a bit with this one. Thanks in advance.
n=3, l=0,
n=2, l=1
Do I just have to say that it has for example one 3s orbital with 3 subshells or do I have to add other information as well? I am struggling a bit with this one. Thanks in advance.
1 Answer
Here's how you can do that.
Explanation:
You have values for three our of the four quantum numbers that we use to describe the location and the spin of an electron inside an atom.
- the principal quantum number,
#n# - the angular momentum quantum number,
#l# - the magnetic quantum number,
#m_l# .
This means that in order to describe the electrons defined by these two incomplete quantum number sets, you must mention
- the energy shell in which the electron is located because you know the value of
#n# - the energy subshell in which you can find the electron because you know the value of
#l# - the orientation of the orbital in which the electron resides because you know the value of
#m_l#
For the first set, you have
#n = 3, l=0, m_l = 0#
This set describes an electron that
- is located in the third energy shell because
#n = 3# - is located in the
#s# subshell because#l = 0# - is located in the
#s# orbital because#m_l = 0#
So for this first electron, you have the third energy shell, the
For the second set, you have
#n = 2, l =1, m_l = 1#
This time, the set describes an electron that
- is located in the second energy shell because
#n = 2# - is located in the
#p# subshell because#l = 1# - is located in one of the three
#p# orbitals because#m_l = 1#
So for this electron, you have the second energy shell, the